Respuesta :
Explanation:
Expression for rate of the given reaction is as follows.
Rate = k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y[/tex]
Therefore, the reaction equations by putting the given values will be as follows.
[tex]1.8 \times 10^{-5} = k[0.105]x [0.15]y[/tex] ............. (1)
[tex]7.2 \times 10^{-5} = k [0.105]x [0.30]y[/tex] ........... (2)
[tex]3.6 \times 10^{-5} = k [0.0525]x [0.30]y[/tex] ............ (3)
Now, solving equations (1) and (2) we get the value of y = 2. Therefore, by solving equation (2) and (3) we get the value of x = 1.
Therefore, expression for rate of the reaction is as follows.
Rate = [tex]k[HgCl_{2}]x [C_{2}O^{2-}_{4}]y[/tex]
Rate = [tex]k [HgCl2]1 [C_{2}O^{-2}_{4}]2[/tex]
Hence, total order = 1 + 2 = 3
According to equation (1),
[tex]1.8 \times 10^{-5} = k[0.105]x [0.15]y[/tex]
[tex]1.8 \times 10^{-5} = k [0.105]1 [0.15]2[/tex]
k = [tex]7.6 \times 10^{-3} M^{-2} min^{-1}[/tex]
Thus, we can conclude that rate constant for the given reaction is [tex]7.6 \times 10^{-3} M^{-2} min^{-1}[/tex].
